In the electrochemical cell: 
  $Zn | ZnS{O}_4 (0.01 M) || CuS{O}_4(1.0 M) | C\mathrm{u, }$the emf of this Daniel cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ is changed to 0.01 M, the emf changes to E₂. From the following, which one is the relationship between E₁ and E₂ ? 
(Given, \(\frac{RT}{F}\) = 0.059)

1. $E_1<E_2$

2. $E_1>E_2$

3. $E_2=0\ne E_1$

4. $E_1=E_2$

The pressure of H₂ required to make the potential of H₂ - electrode zero in pure water at 298 K is

1. 10^-12  atm
2. 10^-10  atm
3. 10^-4  atm
4. 10^-14 atm

The equilibrium constant of the reaction : 
Cu(s) + 2Ag⁺ (aq) → Cu²⁺(aq)+2Ag(s); 
E⁰=0.46 V at 298 K is :

1. $2.4\times {10}^{10}$

2. $2.0\times {10}^{10}$

3. $4.0\times {10}^{10}$

4. $4.0\times {10}^{15}$

A hypothetical electrochemical cell is shown below.
A|A⁺(x M) || B⁺(y M)|B
The Emf measured is +0.20 V. The cell reaction is:

1. A⁺ + B → A + B⁺

2.  A⁺ + e^- → A ; B⁺ + e^- → B

3. The cell reaction cannot be predicted.

4. A + B⁺ → A⁺ + B